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6-2.Equilibrium-II (Ionic Equilibrium)
hard
At ${20\,^o}C,$ the $A{g^ + }$ ion concentration in a saturated solution of $A{g_2}Cr{O_4}$ is $1.5 \times {10^{ - 4}}\,mole/litre.$ At ${20\,^o}C,$the solubility product of $A{g_2}Cr{O_4}$ would be
A
$3.3750 \times {10^{ - 12}}$
B
$1.6875 \times {10^{ - 10}}$
C
$1.6875 \times {10^{ - 12}}$
D
$1.6875 \times {10^{ - 11}}$
Solution
(c) $AgCr{O_4} ⇌ \mathop {2A{g^ + }}\limits_{{{(2S)}^2}} + \mathop {CrO_4^ – }\limits_{S\,\,\,} $
${K_{sp}} = 4{S^3}$ given $2S = 1.5 \times {10^{ – 4}}$
$\therefore \,{K_{sp}} = {(2S)^2} \times S$
$ = {(1.5 \times {10^{ – 4}})^2} \times \left( {\frac{{1.5 \times {{10}^{ – 4}}}}{2}} \right)$ $ = 1.6875 \times {10^{ – 12}}$
Standard 11
Chemistry
